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Arrange the following elements by increasing Ionization energy: He, Ar, Ne, Kr *Item one should be the highest energy, Item 4 should be the lowest

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The arrangement of the elements by increasing ionization energy is; Kr < Ar < Ne < He.

However, If item 1 should be the highest, then we have; He > Ne > Ar > Kr.

The ionization energy of an element is simply defined as the quantity/amount of energy required to completely remove an electron from its outermost shell.

However, periodic trends occur in the periodic table.

  • A relationship exists between the ionization energy of elements in the periodic table and their atomic radii.

In essence, the larger the atomic radii of elements, the lesser is their ionization energy.

  • It is important to note that the atomic radii of elements increases down the group and decreases across the period in the periodic table.

Consequently, inference drawn from the statements above is enough to conclude that elements with smaller atomic radii have higher ionization energy as the electrons are closer to the nucleus and the electrostatic attraction is greater.

Ultimately, the arrangement of the elements by increasing ionization energy is;

  • Kr < Ar < Ne < He.

However, If item 1 should be the highest, then we have;

  • He > Ne > Ar > Kr.

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